How do changes in concentration affect equilibrium shifts?

Changes in concentration can significantly influence the position of equilibrium in a chemical reaction, as described by Le Chatelier's principle. According to this principle, when a system at equilibrium experiences a change in concentration, it will adjust the equilibrium position to counteract that change, aiming to restore a new equilibrium state.

In the context provided, removing a product from a system at equilibrium leads to a shift to the left, which favors the formation of reactants. This shift occurs because, by reducing the concentration of the products, the system reacts to counter the loss of that product by converting some of the reactants back into products. Thus, the equilibrium position moves towards the left to produce more of the product that was removed and restore balance.

This is a fundamental concept in chemical equilibrium, where the system seeks to maintain its equilibrium constant by responding to changes in concentration of either reactants or products.